Acid/Base Titration Lab

    A Bronsted-Lowery acid is any substance that donates a Hydrogen atom, and a Bronsted-Lowery base is substances that accept a Hydrogen atom. All acid base equations have the hydrogen in common whether it is a cation or an anion. Titration is the process of finding the unknown molarity of one solution by slowly adding  a solution of a known concentration to the unknown.

Small Scale Reactions

     In this experiment we tested to see what anions and cations would precipitate when reacted. Then we found the net ionic equations for each reaction, if there was one. Solubility rules played a large part in the experiment. We learned what was soluble in water, and what wasn't. That's why some of the solutions precipitated when reacted, because the solutions created a solid when they reacted. The molecular, ionic, and net ionic formulas can all be found with each other unless you have only the net ionic equation. Here is our experiment sheet for the precipitate reactions.

3rd 3 questions

1. I am understanding the stoich more and more every time we use it, also I understand molarity and molality, and the solutions parts (solute and solvent).
2. I need a bit of work on finding the charges and utilizing them in the net ion equations, but I am getting the hang of finding the charges.
3. I plan on taking notes on charges and doing a few extra steps while finding the net ion equations.

Small Scale Reactions

Using these small scale reactions with the baking soda and carbon dioxide, I can graphically prove the conservation of mass, the stoichiometric relationships, and the limiting reagents.

Water and Electrolytes

A solution is a mixture of a solute and a solvent. An electrolyte is an ionic compound composed of anions and cations that conduct electricity. Here is a particle diagram of the salt solution.

I created two different concentrations of the salt solutions. Here are the qualitative demonstrations of this difference.

                                           My teacher's results                     My results

Beaker 3

Beaker 1

Beaker 2

You can mathematically show the difference in concentration by measuring the amount of electrolytes in each beaker. You can tell which beaker is D.I. water, tap water, or salt water by measuring the amount of electrolytes by putting in the copper wires to see whether it conducts electricity or not. I took advantage of the appearance of the solution and the way it conducted (or didn't conduct) electricity to find out which one was which. I recreated my teacher's results by using D.I. water for no light, tap water for dim light, and D.I. water with a few grams of salt added for bright light. I had an error in my calculations; I had used tap water plus salt at the beginning for beaker 2, but I ended up having D.I. water plus salt for the final trial. The final concentrations were 700ml of D.I. water for beaker 3, 600ml tap water for beaker 1, and 760ml of D.I. water combined with 3.16g of salt for beaker 2. My results came very close compared to my teachers, as shown above.